Consider this system at equilibrium. A(aq)↽−−⇀B(aq)ΔH=+750 kJ/mol A(aq)↽−−⇀B(aq)ΔH=+750 kJ/mol What can be said about Q and K immediately after an increase in temperature? Q < K because Q decreased. Q = K because neither changed. Q < K because K increased. Q > K because K decreased. Q > K because Q increased. How will the system respond to a temperature increase? shift left shift right no change

Q < K because K increased.

Reaction equilibrium shift towards right.

Explanation:

Reaction equilibrium:

For this reaction, is positive. This signifies that the given reaction is endothermic. So, with increase in temperature, reaction equilibrium shift towards right in accordance with Le-chatelier principle.

So, with increase in temperature, more A will be converted to B.

Equilibrium constant in terms of concentration, where [B} and [A} are equilibrium concentrations of B and A respectively.

Hence will increase with increase in temperature.

At equilibrium, Q (reaction quotient) = .

But immediately after an increase in temperature, Q < as is higher in this increased temperature as compared to previous temperature.